Chemistry Unit 4: Valence electrons and the periodic table

What are valence electrons?

Electrons in the atom’s outermost orbitals

What is the electron dot structure

It’s involved in forming chemical bonds

What is periodic law?

The specific periodic repetition of chemical and physical properties of elements when arranged by increasingg the atomic number

What are ←→ rows called

Periods

__ number of electrons for every element in a column

Same

__ number of energy levels for elements in rows

Same

What blocks are Representative elements

S and P block (groups 1, 2, 13-18)

What blocks are transition elements?

D block (groups 3-12)

What blocks are inner transition elements?

F block

What group(s) are alkali metals

Group 1

What group(s) are alkaline earth metals?

Groups 3-12

What group(s) are inner transition metals?

Lanthanide and actinide

What are the properties of metals

hard, solid at room temp, malleable, ductile, loses electrons, shiny, good conductors of heat

What are the properties of non metals?

Upper right on pt, generally gases or brittle solids, poor conductors of heat

What are the properties of metalloids?

Semimetals, staircase on pt, properties are characteristics of both metals and nonmetals

What are the periodic table trends for atomic radius

Increases down and to the left

What is an ion?

A charged particle

How does a neutral atom form a positive ion?

It loses an electron

What is ionization energy?

Energy required to remove an electron from a gaseous atom

Atoms with high ionization energy are likely or unlikely to form positive ions?

Unlikely

Ionization energy increases to the ___

right

Ionization energy increases going __ the periodic table

up

What is electronegativity?

The relative ability of an atom to attract electrons in a chemical bond

Electronegativity increases as you move __ the periodic table

up

Electronegativity increases as you move to the ___

right

___ and ___ have the same periodic table trends

Ionization energy and electronegativity